Abstract
THE composition of chlorine hydrate has been the subject of much experimental work. Faraday, by analysis, found the composition to be Cl2.10H2O. The composition has also been determined analytically by Roozeboom1 who found Cl2.8H2O, Bouzat and Azinires2 who found Cl2.6H2O, and more recently by Anwar-Ullah3 who agreed with this last formula. De Forcrand4 used an empirical rule to calculate the number of molecules of water present. According to de Forcrand's rule, if b.Delta;H is the heat of dissociation of the hydrate into gaseous chlorine and ice, and T the temperature at which the dissociation pressure is 760 mm., then b.Delta;H/T is a constant the value of which is approximately 30. The value of T is known from the dissociation pressures determined experimentally by Roozeboom, and this gives a value ofb.Delta;H equal to 8,478 cal./gm. mol. Since de Forcrand's rule is only an approximation, this value of b.Delta;H is very inaccurate. De Forcrand determined the heat of dissociation of the hydrate into gaseous chlorine and water by measuring the heat of solution of the hydrate in water and obtained a value of 18,360 cal. /gm. mol. The number of molecules of water present in the hydrate is then given by n = 18, 360 8, 478/1,436 = 6. 88, the latent heat of fusion of ice being 1,436 cal./gm. mol. De Forcrand therefore assumed the composition to be Cl2.7H2O.
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References
Roozeboom, Rec. Trav. Chim., 3, 68, 1884; 4, 65, 1885.
Bouzat and Azinières, C.R., 77, 1444 (1923).
Anwar-Ullah, J. Chem. Soc., 1172 (1932).
De Forcrand, C.R., 133, 1304 (1901); 134, 743, 768, 835, 991 (1902).
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HARRIS, I. Composition of Chlorine Hydrate. Nature 151, 309 (1943). https://doi.org/10.1038/151309a0
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DOI: https://doi.org/10.1038/151309a0
Santiago Schepens
This is an incomplete reference and the conclusion is, therefore, erroneous. It's lacking the last paragraph of Harris´ original article from 1943 which ends: "(...); and there is little doubt, therefore, that the correct formula is Cl2.8H2O."